24. A 25.0 mL volume of a 0.200 M N,H& solution (K 1.70x10 titrated to the equivalence point with 0.100 M HCl....

Question

Question

Answer 1

Answer #1

b 2 Dom x 2S.ow Ve) Aa ㅓん 6c.nl t e) 5

> Shouldn’t the answer be 8.23 since 5.77 is the pOH (because we used Kb instead of Ka)?

Bella Moen Sat, Nov 13, 2021 8:40 PM

Answer 2

Similar Homework Help Questions

A 25.0 mL volume of a 0.200 M N2H4 solution (Kb = 1.70 × 10−6) is...

A 25.0 mL volume of a 0.200 M N2H4 solution (Kb = 1.70 × 10−6) is titrated to the equivalence point with 0.100 M HCl. What is the pH of this solution at the equivalence point? The titration is: N2H4 + HCl N2H5+ + Cl−
19. The conjugate base salt to a weak acid (NaA) is titrated with 0.100 M HCl...

19. The conjugate base salt to a weak acid (NaA) is titrated with 0.100 M HCl to its equivalence point. A 25.0 mL solution of a 0.200 M solution of the salt was titrated. The pK, for the unknown conjugate acid is 4.31. (a) Will the equivalence point be acidic or basic for this titration? i.e. pH less than 7.0 or greater than 7.0? (b) What is the volume in mL needed of HCl to reach the equivalence point? (c)...
Consider the titration of a 25.0 mL sample of 0.100 M HCl with 0.200 M KOH....

Consider the titration of a 25.0 mL sample of 0.100 M HCl with 0.200 M KOH. The volume of equivalence is 12.50 mL. (Remember to report pH values with two places past the decimal point.) A)What is the pH of the sample before any KOH is added? B)What is the pH after 9.00 mL of KOH have been added? C)What is the pH at the equivalence volume? D)What is the pH after the addition of 14.0 mL of KOH?

A 25.0 mL volume of a 0.200 M N2H4 solution (Kb = 1.70 x 10-6) is...

A 25.0 mL volume of a 0.200 M N2H4 solution (Kb = 1.70 x 10-6) is titrated to the equivalence point with 0.100 M HCl. What is the pH of this solution at the equivalence point? The titration is: N2H4 + HCI= N2H5+ + C1- * O rö oo O ö in O ü o O ö O e. 7.00 Consider the following Bronsted-Lowery acid-base reaction: HCIO2 + N(CH3)3 = [HN(CH3)3]* + C1025 Which two substances represent Bronsted-Lowery bases in...
1. Consider the titration of 50.0 mL of 0.200 M HNO3 with 0.100 M NaOH solution....

1. Consider the titration of 50.0 mL of 0.200 M HNO3 with 0.100 M NaOH solution. What volume of NaOH is required to reach the equivalence point in the titration? a. 25.0 mL b. 50.0 mL c. 1.00 × 10^2 mL d. 1.50 × 10^2 mL 2. Consider the following acid–base titrations: I) 50 mL of 0.1 M HCl is titrated with 0.2 M KOH. II) 50 mL of 0.1 M CH3COOH is titrated with 0.2 M KOH. Which statement...
Two 25.0 mL samples of one 0.100 M HCl and the other 0.100 M HF were...

Two 25.0 mL samples of one 0.100 M HCl and the other 0.100 M HF were titrated with 0.200 M KOH answer each of the following questions regarding these two titrations Two 25.0 mL samples, one 0.100 M HCl and the other 0.100 M HF, were titrated with 0.200 M KOH. Answer each of the following questions regarding these two titrations You may want to reference (Pages 755 - 769) Section 17.4 while completing this problem. Part A What is...

a 50.0 mL sample of a 0.100 M solution of NaCN is titrated by 0.100 M...

a 50.0 mL sample of a 0.100 M solution of NaCN is titrated by 0.100 M HCl. kb for CN is 2.0x10-5. A.calculate the pH of the solution prior to the start of the titration. B after the addition of 10.0 mL. C. after the addition of 25.0 mL of 0.100 M HCl. D. at the equivalence point. E. after the addition of 60.0 mL of 0.100 M HCl
Two 25.0 mL samples, one 0.100 M HCl and the other 0.100 M HF, were titrated...

Two 25.0 mL samples, one 0.100 M HCl and the other 0.100 M HF, were titrated with 0.200 M KOH. Answer each of the following questions regarding these two titrations. Part A What is the volume of added base at the equivalence point for HCl? Part B What is the volume of added base at the equivalence point for HF? Express your answer in milliliters.
1. 25.0 mL of a 0.100 M solution of NH, is titrated with 0.150M HCl. After...

1. 25.0 mL of a 0.100 M solution of NH, is titrated with 0.150M HCl. After 10.0 mL of the HCl has been added, the resultant solution is: A) Basic and before the equivalence point B) Basic and after the equivalence point C) Acidic and before the equivalence point D) Acidic and after the equivalence point E) Neutral and at the equivalence point

Two 22.0 mL samples, one 0.100 M HCl and the other 0.100 M HF, were titrated...

Two 22.0 mL samples, one 0.100 M HCl and the other 0.100 M HF, were titrated with 0.200 M KOH. Answer each of the following questions regarding these two titrations. a) What is the volume of added base at the equivalence point for HCl? b)What is the volume of added base at the equivalence point for HF? c)Predict whether the pH at the equivalence point for each titration will be acidic, basic, or neutral. neutral for HF, and basic for...